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Worksheet: Osmotic Concentration

Q1:

The osmotic pressure of human blood is 7.6 atm at 3 7 C . What mass of glucose, C H O 6 1 2 6 , is required to make 1.00 L of aqueous solution for intravenous feeding if the solution must have the same osmotic pressure as blood at body temperature, 3 7 C ?

Q2:

A 0.010 M solution of the weak acid H A has an osmotic pressure of 0.293 atm at 2 5 C . A 0.010 M solution of the weak acid H B has an osmotic pressure of 0.345 atm under the same conditions. Each solution contains three dissolved species: the weak acid ( H A or H B ), the conjugate base ( A or B ), and the hydrogen ion ( H + ). The osmotic pressure of each solution is related to the solute concentrations in molar units.

Which acid has the larger equilibrium constant for ionization, H A ( H A ( ) A ( ) + H ( ) ) a q a q a q + or H B ( H B ( ) H ( ) + B ( ) ) a q a q a q + ?

  • A H A
  • B H B

What is the equilibrium constant for the ionization of H A ?

  • A 5 × 1 0 4
  • B 6 × 1 0 5
  • C 4 × 1 0 4
  • D 3 × 1 0 3
  • E 3 × 1 0 2